$2SO_3 \rightleftharpoons 2SO_2 + O_2$. Initially,$3$ moles of $SO_3$ were heated. If the degree of dissociation of $SO_3$ is $40\%$,find the total number of moles at equilibrium.

The vapor density of a gas is $35.5$. What is the volume occupied by $3.55 \, g$ of this gas at $N.T.P$?

Gaseous $N_2O_4$ dissociates into gaseous $NO_2$ according to the reaction:
$N_2O_{4(g)} \rightleftharpoons 2NO_{2(g)}$
At $300 \ K$ and $1 \ atm$ pressure,the degree of dissociation of $N_2O_4$ is $0.2$. If one mole of $N_2O_4$ gas is contained in a vessel,then the density of the equilibrium mixture is.......$g/L$

$0.1 \ mol$ of $H_2S_{(g)}$ is kept in a $0.4 \ L$ vessel at $1000 \ K$. For the reaction $2 H_2S_{(g)} \rightleftharpoons 2 H_{2(g)} + S_{2(g)}$,$K_c = 10^{-6}$. The percentage dissociation of $H_2S$ is.......$\%$

The degree of dissociation of $PCl_5$ $(\alpha)$ obeying the equilibrium,$PCl_5 \rightleftharpoons PCl_3 + Cl_2$,is approximately related to the pressure at equilibrium by (given $\alpha << 1$):

The density of air is $0.00130 \ g/mL$. The vapour density of air will be